Designing a galvanic cell. Write ancedequation for thehalf-reaction thathappens at theanode.Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.Do you haveenoughinformation tocalculate the cellvoltage understandardconditions?If you said it waspossible tocalculate the cellvoltage, do so and0YesNoenter your answer OVhere. Be sure youranswer has thecorrect number ofsignificant digits. A chemist designs a galvanic cell that uses these two half-reactions:MnO4(aq) + 2 H₂O(1)+3eWrite a balancedequation for thehalf-reaction thathappens at thecathode.Write a balancedequation for thehalf-reaction thathappens at theanode.Answer the following questions about this cell.Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.half-reaction3+2+Fe³+ (aq) + e → Fe (aq)Do you haveenoughinformation tocalculate the cellvoltage understandardconditions?0OMnO2(s)+4 OH (aq)YesNostandard reduction potentialE=+0.59 VEd=+0.771 V"red

The question is based on the concept of electrochemistry . We have to write reactions taking place…

Write anced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of cignific digito 0 Yes No Ov

Write anced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of cignific digito 0 Yes No Ov

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Designing a galvanic cell.

Write anced
equation for the
half-reaction that
happens at the
anode.
Write a balanced
equation for the
overall reaction
that powers the
cell. Be sure the
reaction is
spontaneous as
written.
Do you have
enough
information to
calculate the cell
voltage under
standard
conditions?
If you said it was
possible to
calculate the cell
voltage, do so and
0
Yes
No
enter your answer OV
here. Be sure your
answer has the
correct number of
significant digits.

A chemist designs a galvanic cell that uses these two half-reactions:
MnO4(aq) + 2 H₂O(1)+3e
Write a balanced
equation for the
half-reaction that
happens at the
cathode.
Write a balanced
equation for the
half-reaction that
happens at the
anode.
Answer the following questions about this cell.
Write a balanced
equation for the
overall reaction
that powers the
cell. Be sure the
reaction is
spontaneous as
written.
half-reaction
3+
2+
Fe³+ (aq) + e → Fe (aq)
Do you have
enough
information to
calculate the cell
voltage under
standard
conditions?
0
O
MnO2(s)+4 OH (aq)
Yes
No
standard reduction potential
E=+0.59 V
Ed=+0.771 V
"red

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